The Haber process is used to produce ammonia from nitrogen and hydrogen gases: N

Question

The Haber process is used to produce ammonia from nitrogen and hydrogen gases:

N2(g)+3H2(g) -> 2NH3(g) Delta H = -92.4kJ

What will the effect on the final equilibrium amount of NH3(g) (whether it be more or less) be if a gaseous mixture originally at equilibrium at 298K is subjected to the following changes: Please explain why also.

a) more H2 is added

b)a catalyst is added

c)the mixture is transferred to a reaction vessel of greater volume

d) the partial pressure of N2 is decreased

e) the temperature is lowered to 273K

f) the partial pressure of NH3 is decreased.

Explanation / Answer

N2(g)+3H2(g) -> 2NH3(g) Delta H = -92.4kJ

a) more H2 is added : Equilibrium shifts right side.so that amount of NH3 increases.

b)a catalyst is added : No effect on equilibrium.

c)the mixture is transferred to a reaction vessel of greater volume : Equilibrium shifts left side.so that amount of NH3 decreases.

d) the partial pressure of N2 is decreased : Equilibrium shifts left side.so that amount of NH3 decreases.

e) the temperature is lowered to 273K : Equilibrium shifts right side.so that amount of NH3 increases.

f) the partial pressure of NH3 is decreased. : Equilibrium shifts right side.so that amount of NH3 increases.

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